Homework Answers
2HCl(aq) + CaCO3(s) -------------> CaCl2(aq) + CO2(g) + H2O(l)
1 mole of CO2 produce from 1 mole of HCl react with excess of CaCo3
22.4L of CO2 produce from 1 mole of HCl react with excess of CaCO3
32.0L of CO2 produced from = 1*32/22.4 = 1.43mole of HCl
no of moles HCl = molairty * volume in L
1.43 = 0.75* volume in L
volume in L = 1.43/0.75 = 1.91L >>>>>answer
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i need the answer for part 2 and 3! please
PART II - Short answer questions...
2. What is the percent yield of CO2 (44.01 g/mol) if 0.275 g of carbon dioxide...
2. What is the percent yield of CO2 (44.01 g/mol) if 0.275 g of carbon dioxide is obtained by heating 1.75 g of calcium carbonate, CaCO3 (100.09 g/mol)? (10 points) show all setup & work CaCO3) + CaO) + CO2Q Answer: % yield = A MULA needed to react with excess CaCO3 to produce 32.0 L of CO2 at S
Please answer the questions clearly, showing all working. 1(i). Balance the following equations, and then write...
Please answer the questions clearly, showing all working. 1(i). Balance the following equations, and then write the net ionic equation (a) (NH4)2CO3(aq) + Cu(NO3)2(aq) → CuCO3(s) + NH4NO3(aq) (b) Mg(OH)2(s) + HCl(aq) → MgCl2(aq) + H2O(l) (c) BaCO3(s) + HBr(aq) → BaBr2(aq) + H2O(l) + CO2(g) 1(ii). For each reaction equation, identify the driving force of the reaction 2. What is an electrolyte? How can you experimentally differentiate between a weak electrolyte and a strong electrolyte? Name and give the...
2. Consider the given reaction, and use all your stoichiometry skills to answer the three-part question....
2. Consider the given reaction, and use all your stoichiometry skills to answer the three-part question. For both parts, show your math work, round your final answers to 3 significant figures and circle them. __Mg (s) + ___ HCl (aq) → __MgCl2 (aq) + _H2 (g) a) If 8.0 grams of Mg is used with excess HCI, what mass of HCI will react? (10 points) b) If 8.0 grams of Mg is used with excess HCI, what mass of H2...
Answer: volume in L = 3. How many liters of 0.750 M HCl are needed to react with excess CaCO3 to produce 32.0 L of...
Answer: volume in L = 3. How many liters of 0.750 M HCl are needed to react with excess CaCO3 to produce 32.0 L of CO2 at STP? (10 points) show all setup &work 2HCI(ag)+CaCO3) CaCl2(ag) + CO2@ +H20( Answer: volume of HCl =
all please, no mid way answers because then i dont get the help necessary. Name 2)...
all
please, no mid way answers because then i dont get the help
necessary.
Name 2) Nitrogen dioxide gas reacts with water to form nitric acid and nitrogen monoxide gas a) Write a balanced chemical equation for the reaction. b) If 5.Og nitrogen dioxide completed reacted, how many grams of nitric acid would form? c) If 5.0g water completed reacted, how many grams of nitric acid would form? d) What is the limited reagent? nitrogen dioxide, NO2 e) If 5.0g...
balance each of the following equations Fall 209 CHM 105.004 Exam 2 Answer all the question in order in the blue b...
balance each of the following equations
Fall 209 CHM 105.004 Exam 2 Answer all the question in order in the blue book. Plesse leave at least two lines between question and show your calculations for full credit. N-6.023 x 10” particles per mol: R 0.08.205 L-atm/(mol-K) b) Al2(PO4) 3 e) CuSO4-5 H2O 1. Calculate the molar masses of: a) (NH4)2SO4 2. Calculate: a) the number of atoms of calcium in a 10.50 g sample of the metal b) the mass...
please answer these 3 questions 1. 2. 3. Part A Ammonia can also be synthesized by...
please answer these 3 questions
1. 2.
3.
Part A Ammonia can also be synthesized by the reaction: 3H2(g) + N2(g) +2NH3(g) What is the theoretical yield of ammonia, in kilograms, that we can synthesize from 5.27 kg of H2 and 34.9 kg of N2? VAED ? theoretical yield of NH3 = kg Submit Request Answer Review | Constants I Periodic lable Mining companies use this reaction to obtain iron from iron ore: Fe2O3(s) +3CO(g) + 2Fe(s) + 3CO2(g) Part...
Answer the question in below. Answer all 4 parts, and please show your calculation, and explain...
Answer the question in below. Answer all 4 parts, and please
show your calculation, and explain a bit.
1. For the hydrolysis of sulfamic acid NH,SO3H (MW 97.1 g.mol-') reacting with Ba(NO3) (MW 261.34 g.mol-') to produce BaSO4 (MW 233.38 g.mol"), we use a solution containing 1.50 g Ba(NO3)2 and 2.50 g of NH2SO3H: Ba(NO3)2(aq) + NH2SO3H(aq) + H20 (1) - BaSO4(s) + NH4NO3(aq) + HNO3(aq) (a) Use the expression below and calculate the grams of sulfamic acid needed to...
Could someone please answer this?! I’ve been waiting for my other one for almost 5 hours...
Could someone please answer this?! I’ve been waiting for my
other one for almost 5 hours .
c) Calculate your actual yield of sodium acetate (in grams): Mass of reaction (#3) sodium acetate mass of beaker after the reaction (#9)- mass of beaker and boiling stones before Actual yield of sodium acetate Use your actual yield of sodium acetate and your theoretical yield (in grams) of sodium acetate to calculate the percent yield for the reaction (formula from page 1)....
Please show all steps and explain, as I need to understand for an exam. Thx! 14....
Please show all steps
and explain, as I need to understand for an exam. Thx!
14. The combustion of a hydrocarbon produces 66.02 g CO2 (molecular weight 44.01 g/mol) and 13.51 g H2O (molecular weight 18.01 g/mol). It's empirical formula must be: A. CH B. C2H C. CH2 D. C3H2 E. none of the above. ANSWER: A
2. What is the percent yield of CO2 (44.01 g/mol) if 0.275 g of carbon dioxide is obtained by heating 1.75 g of calcium carbonate, CaCO3 (100.09 g/mol)? (10 points) show all setup & work CaCO3) + CaO) + CO2Q Answer: % yield = A MULA needed to react with excess CaCO3 to produce 32.0 L of CO2 at S
2. Consider the given reaction, and use all your stoichiometry skills to answer the three-part question. For both parts, show your math work, round your final answers to 3 significant figures and circle them. __Mg (s) + ___ HCl (aq) → __MgCl2 (aq) + _H2 (g) a) If 8.0 grams of Mg is used with excess HCI, what mass of HCI will react? (10 points) b) If 8.0 grams of Mg is used with excess HCI, what mass of H2...
Answer: volume in L = 3. How many liters of 0.750 M HCl are needed to react with excess CaCO3 to produce 32.0 L of CO2 at STP? (10 points) show all setup &work 2HCI(ag)+CaCO3) CaCl2(ag) + CO2@ +H20( Answer: volume of HCl =
all
please, no mid way answers because then i dont get the help
necessary.
Name 2) Nitrogen dioxide gas reacts with water to form nitric acid and nitrogen monoxide gas a) Write a balanced chemical equation for the reaction. b) If 5.Og nitrogen dioxide completed reacted, how many grams of nitric acid would form? c) If 5.0g water completed reacted, how many grams of nitric acid would form? d) What is the limited reagent? nitrogen dioxide, NO2 e) If 5.0g...
balance each of the following equations
Fall 209 CHM 105.004 Exam 2 Answer all the question in order in the blue book. Plesse leave at least two lines between question and show your calculations for full credit. N-6.023 x 10” particles per mol: R 0.08.205 L-atm/(mol-K) b) Al2(PO4) 3 e) CuSO4-5 H2O 1. Calculate the molar masses of: a) (NH4)2SO4 2. Calculate: a) the number of atoms of calcium in a 10.50 g sample of the metal b) the mass...
please answer these 3 questions
1. 2.
3.
Part A Ammonia can also be synthesized by the reaction: 3H2(g) + N2(g) +2NH3(g) What is the theoretical yield of ammonia, in kilograms, that we can synthesize from 5.27 kg of H2 and 34.9 kg of N2? VAED ? theoretical yield of NH3 = kg Submit Request Answer Review | Constants I Periodic lable Mining companies use this reaction to obtain iron from iron ore: Fe2O3(s) +3CO(g) + 2Fe(s) + 3CO2(g) Part...
Answer the question in below. Answer all 4 parts, and please
show your calculation, and explain a bit.
1. For the hydrolysis of sulfamic acid NH,SO3H (MW 97.1 g.mol-') reacting with Ba(NO3) (MW 261.34 g.mol-') to produce BaSO4 (MW 233.38 g.mol"), we use a solution containing 1.50 g Ba(NO3)2 and 2.50 g of NH2SO3H: Ba(NO3)2(aq) + NH2SO3H(aq) + H20 (1) - BaSO4(s) + NH4NO3(aq) + HNO3(aq) (a) Use the expression below and calculate the grams of sulfamic acid needed to...
Could someone please answer this?! I’ve been waiting for my
other one for almost 5 hours .
c) Calculate your actual yield of sodium acetate (in grams): Mass of reaction (#3) sodium acetate mass of beaker after the reaction (#9)- mass of beaker and boiling stones before Actual yield of sodium acetate Use your actual yield of sodium acetate and your theoretical yield (in grams) of sodium acetate to calculate the percent yield for the reaction (formula from page 1)....
Please show all steps
and explain, as I need to understand for an exam. Thx!
14. The combustion of a hydrocarbon produces 66.02 g CO2 (molecular weight 44.01 g/mol) and 13.51 g H2O (molecular weight 18.01 g/mol). It's empirical formula must be: A. CH B. C2H C. CH2 D. C3H2 E. none of the above. ANSWER: A
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