1.
5.00 g of butane are combusted in a sealed container containing 2.00 g of oxygen gas. The balanced reaction for the combustion of butane is shown below. How many grams of the excess reagent are left over? (This question first requires you to determine the limiting reagent, and then calculate how much will be leftover). Pease answer in g.
Molar Mass Butane: 58.12 g/mol
Molar Mass Oxygen Gas: 32.0 g/mol
2CH3CH2CH2CH3 + 13O2 --> 8CO2 + 10H2O
2.
If 10.0 g HCl is reacted with excess NaOH and 12.0 g of NaCl is produced, what is the percent yield of the reaction?
HCl + NaOH --> H2O + NaCl
1. 5.00 g of butane are combusted in a sealed container containing 2.00 g of oxygen...
2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g) A)Calculate the mass of water produced when 3.48 g of butane reacts with excess oxygen. B)Calculate the mass of butane needed to produce 92.0 g of carbon dioxide.
4) If 300.0 g of butane were completely combusted in the presence of excess oxygen, what mass of CO2 would be produced?
1.)) An unknown compound containing carbon, hydrogen and oxygen is combusted. If 25.000 g of the compound produced 61.024 g of CO2 and 24.981 g of H2O, what is the empirical formula of the compound? 2.)) If the molar mass of this compound is 72.1 g/mol, what is the molecular formula?
A sample of 8.77 g of liquid 1-propanol, C,H, O, is combusted with 40.8 g of oxygen gas. Carbon dioxide and water are the products Write the balanced chemical equation for the reaction. Physical states are optional. chemical reaction: What is the limiting reactant? O oxygen O 1-propanol How many grams of CO, are released in the reaction? mass of CO How many grams of the excess reactant remain after the reaction is complete? mass of excess reactant remaining:
A sample of 5.61 g of liquid 1‑propanol, C3H8O, is combusted with 36.8 g of oxygen gas. Carbon dioxide and water are the products. Write the balanced chemical equation for the reaction. Physical states are optional. chemical reaction: How many grams of CO2 are released in the reaction? mass of CO2: g How many grams of the excess reactant remain after the reaction is complete? mass of excess reactant remaining: g
8. How many gram Na in 5.00g Na2SO4? A. 0.035 g B. 1.31 g C. 1.62 g D. 0.97 g E. 0.81 g 9. A compound containing only carbon and hydrogen has 85.7 wt% C and 14.3 wt%H. Its molar mass is 56 amu. What is its molecular formula? A. C4H8 B. C2H4 C. C2H D. CH2 E. CH 10. Balance the following reactions. No fractional coefficients, coefficients must be the lowest whole numbers. a) ____K + ____H2O →...
For this reaction, 26.0 g iron reacts with 6.11 g oxygen gas. iron (s) + oxygen (g) iron(II) oxide (s) What is the maximum mass of iron(II) oxide that can be formed? g What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete?
A 2.50 g sample of ethanol, C2H5OH, was combusted in the presence of excess oxygen in a bomb calorimeter containing 2.00 kg of water. The temperature of the water increased from 22.500oC to 27.845oC. The heat capacity of the calorimeter is 2520 J/oC and the specific heat capacity of water is 4.184 J/goC. Calculate the molar enthalpy of the combustion reaction in kJ/mol
Consider the reaction below. What is the limiting reactant when 52.0 g of ethene (C2H4, molar mass = 28.0 g/mol) and 128 g of oxygen (molar mass = 32.0 g/mol) are reacted? C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(g) • CO2 Not the correct answer • H2O • C2H4 • O2 what I think is the answer, but I have doubts
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...