Homework Answers
1)
Given:
P = 1.41 atm
V = 567.6 mL
= (567.6/1000) L
= 0.5676 L
T = 22.3 oC
= (22.3+273) K
= 295.3 K
find number of moles using:
P * V = n*R*T
1.41 atm * 0.5676 L = n * 0.08206 atm.L/mol.K * 295.3 K
n = 3.303*10^-2 mol
Molar mass of CO2,
MM = 1*MM(C) + 2*MM(O)
= 1*12.01 + 2*16.0
= 44.01 g/mol
use:
mass of CO2,
m = number of mol * molar mass
= 3.303*10^-2 mol * 44.01 g/mol
= 1.454 g
Answer: 1.45 g
Only 1 question at a time please
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QUESTION 1 0.5 points Save Answer A 567.6 mL sample of carbon dioxide gas, CO2, is...
question 1-4 please :) A sample of nitrogen gas is sealed into a 14.7L container at...
question 1-4 please :)
A sample of nitrogen gas is sealed into a 14.7L container at 426 torr and 106 2 °C How many nitrogen molecules are in the container? {Enter your value in E-notation with three significant figures.] QUESTION 2 A 567.6 ml sample of carbon dioxide gas, CO2, is collected at 1.41 atm and 22.3°C. What is the mass of the carbon dioxide? QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for...
3&4 QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for...
3&4
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) 2 Na(s) + 3 N2(g) Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 30.3 L of N2(g) at 25.6 C and 1 00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water 2 H2(g) O2(a)-2 H20(g) How many grams of water could be produced by...
QUESTION 1 What will be the pressure of 52.5 grams of oxygen gas in a glass...
QUESTION 1 What will be the pressure of 52.5 grams of oxygen gas in a glass container with a volume of 6 L at 15.4 °C? QUESTION 2 At what temperature in °C does 37.34 g of oxygen gas occupy 18.17 L at 622 mm Hg? QUESTION 3 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g)O2(g)-»2 H20(g) How many grams of water could be produced by the reaction of 5.1 liters of hydrogen with...
Please help with these two questions 1.) Consider the reaction between hydrogen gas and oxygen gas...
Please help with these two questions
1.) Consider the reaction between hydrogen gas and oxygen gas to
form water:
2 H2(g) + O2(g) → 2 H2O(g).
How many grams of water could be produced by the reaction of
4.28 liters of hydrogen with 4.11 liters of oxygen at STP?
2.) Automobile airbags use the decomposition of sodium azide,
NaN3, to provide gas for rapid inflation:
2 NaN3(s) → 2 Na(s) + 3 N2(g).
Using stoichiometry and the ideal gas law,...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) → 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 27.2 L of N2(g) at 44 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H20(9). How many grams of water could be...
answer both questions pls!! QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to...
answer both questions pls!!
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) + 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 45.7 L of N2(g) at 41.4 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H2O(g). How many grams...
Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2...
Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) – 2 Na(s) + 3 N2(9). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 20 L of N2(g) at 38 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) → 2 H2O(g). How many grams of water could be produced by...
QUESTION 1 A sample of nitrogen gas is sealed into a 18.6 L container at 715.2...
QUESTION 1 A sample of nitrogen gas is sealed into a 18.6 L container at 715.2 torr and 146.8 °C. How many nitrogen molecules are in the container? (Enter your value in E-notation with three significant figures.] QUESTION 2 A sample of carbon monoxide gas occupies a volume of 200 mL at a pressure of 551.9 torr and a temperature of 633 K. What would its temperature be if the volume were changed to 84 mL at a pressure of...
DO ALL PARTS OF THE QUESTION AND USE SIGNIFICANT FIGURES!!! IF YOU DO NOT DO THIS...
DO ALL PARTS OF THE QUESTION AND USE SIGNIFICANT FIGURES!!! IF
YOU DO NOT DO THIS I WILL DOWNVOTE YOU!!!!
QUESTION 3 2 points Save Answer Automobile airbags are inflated by the rapid decomposition of sodium azide (NaN3). 2 NaN3(s) --> 2 Na(s) + 3 N2(g) What volume of N2 gas, at 0.984 atm and 20.3 °C, is produced by the complete decomposition of 127.6 g of sodium azide? V= __L QUESTION 4 1 points Save Answer What is the...
Please help with these questions 1. Methane (CH4) burns in air to form carbon dioxide and...
Please help with these questions
1. Methane (CH4) burns in air to form carbon dioxide
and water as shown below.
CH4(g) + 2 O2(g) → CO2(g) + 2
H2O(l)
If a sample of methane occupies 802. mL at 3.23 atm, what
pressure (in atm) of oxygen gas with the same temperature and
volume is required to complete the reaction?
2. Consider the reaction between hydrogen gas and nitrogen gas
to form ammonia:
3 H2(g) + N2(g) → 2 NH3(g).
What...
question 1-4 please :)
A sample of nitrogen gas is sealed into a 14.7L container at 426 torr and 106 2 °C How many nitrogen molecules are in the container? {Enter your value in E-notation with three significant figures.] QUESTION 2 A 567.6 ml sample of carbon dioxide gas, CO2, is collected at 1.41 atm and 22.3°C. What is the mass of the carbon dioxide? QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for...
3&4
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) 2 Na(s) + 3 N2(g) Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 30.3 L of N2(g) at 25.6 C and 1 00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water 2 H2(g) O2(a)-2 H20(g) How many grams of water could be produced by...
QUESTION 1 What will be the pressure of 52.5 grams of oxygen gas in a glass container with a volume of 6 L at 15.4 °C? QUESTION 2 At what temperature in °C does 37.34 g of oxygen gas occupy 18.17 L at 622 mm Hg? QUESTION 3 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g)O2(g)-»2 H20(g) How many grams of water could be produced by the reaction of 5.1 liters of hydrogen with...
Please help with these two questions
1.) Consider the reaction between hydrogen gas and oxygen gas to
form water:
2 H2(g) + O2(g) → 2 H2O(g).
How many grams of water could be produced by the reaction of
4.28 liters of hydrogen with 4.11 liters of oxygen at STP?
2.) Automobile airbags use the decomposition of sodium azide,
NaN3, to provide gas for rapid inflation:
2 NaN3(s) → 2 Na(s) + 3 N2(g).
Using stoichiometry and the ideal gas law,...
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) → 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 27.2 L of N2(g) at 44 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H20(9). How many grams of water could be...
answer both questions pls!!
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) + 2 Na(s) + 3 N2(g). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 45.7 L of N2(g) at 41.4 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) + 2 H2O(g). How many grams...
Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation: 2 NaN3(s) – 2 Na(s) + 3 N2(9). Using stoichiometry and the ideal gas law, calculate the mass (in g) of NaN3 required to provide 20 L of N2(g) at 38 °C and 1.00 atm? QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water: 2 H2(g) + O2(g) → 2 H2O(g). How many grams of water could be produced by...
QUESTION 1 A sample of nitrogen gas is sealed into a 18.6 L container at 715.2 torr and 146.8 °C. How many nitrogen molecules are in the container? (Enter your value in E-notation with three significant figures.] QUESTION 2 A sample of carbon monoxide gas occupies a volume of 200 mL at a pressure of 551.9 torr and a temperature of 633 K. What would its temperature be if the volume were changed to 84 mL at a pressure of...
DO ALL PARTS OF THE QUESTION AND USE SIGNIFICANT FIGURES!!! IF
YOU DO NOT DO THIS I WILL DOWNVOTE YOU!!!!
QUESTION 3 2 points Save Answer Automobile airbags are inflated by the rapid decomposition of sodium azide (NaN3). 2 NaN3(s) --> 2 Na(s) + 3 N2(g) What volume of N2 gas, at 0.984 atm and 20.3 °C, is produced by the complete decomposition of 127.6 g of sodium azide? V= __L QUESTION 4 1 points Save Answer What is the...
Please help with these questions
1. Methane (CH4) burns in air to form carbon dioxide
and water as shown below.
CH4(g) + 2 O2(g) → CO2(g) + 2
H2O(l)
If a sample of methane occupies 802. mL at 3.23 atm, what
pressure (in atm) of oxygen gas with the same temperature and
volume is required to complete the reaction?
2. Consider the reaction between hydrogen gas and nitrogen gas
to form ammonia:
3 H2(g) + N2(g) → 2 NH3(g).
What...
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