Given the reaction below, answer the following questions. (30 pts) CH4(g) + S(g) ----> CS2 (g)...
Given the reaction below, answer the following questions. (30 pts) CH4(g) + S(g) ----> CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? ___________ Show charges. C.Given 3.841x1025 molecules of CH4, how many moles is this? D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0oC and 1.25 atm? F.What would be the volume(L) of H2S gas (from Part E above) if the temperature was raised to 125oC(pressure stays the same)?
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Given the reaction below, answer the following questions. (30
pts) CH4(g) + S(g) ----> CS2 (g)...
6. Given the reaction below, answer the following questions. (30 pts) CH(9) + S(g) → CS2...
6. Given the reaction below, answer the following questions. (30 pts) CH(9) + S(g) → CS2 (9) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? Show charges C.Given 3.841x1025 molecules of CH4, how many moles is this? D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0°C and 1.25 atm? F.What would be the volume(L)...
6. Given the reaction below, answer the following questions. (30 pts) CH4(g) + S(g) → CS2...
6. Given the reaction below, answer the following questions. (30 pts) CH4(g) + S(g) → CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? C.Given 3.841x1025 molecules of CH4, how many moles is this? Show charges D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0°C and 1.25 atm? F.What would be the volume(L)...
CH4(9) + S(g) → CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized...
CH4(9) + S(g) → CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? C.Given 3.841x1025 molecules of CH4, how many moles is this? Show charges. D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0°C and 1.25 atm? F.What would be the volume(L) of H2S gas (from Part E above) if the temperature was...
Use the balanced reaction below to answer the following question. Al4C3(s) + 12 H2O(l) → 4 Al(OH)3(s) + 3 CH4(g) Given 6...
Use the balanced reaction below to answer the following question. Al4C3(s) + 12 H2O(l) → 4 Al(OH)3(s) + 3 CH4(g) Given 6.99 grams of Al4C3 and 7.78 grams of H2O, calculate the number of grams of Al(OH)3 that are produced.
answer all questions ral Chemistry Concept 5 pts Question 1 Balance the chemical equation shown below,...
answer all questions
ral Chemistry Concept 5 pts Question 1 Balance the chemical equation shown below, Indicate the stoichiometric coefficients for the reaction. Do not leave answer spaces blank if the coefficient is one (1). AIBrg(aq)+ HBr(aq)- Al(s)+ H2(g) The balanced equation will then be used in the following two questions. 5 pts Question 2 Using the balanced chemical equation from the previous question, how many moles of H2(g) will be formed from 6.24 moles of HBr. Your answer will...
6. Given the reaction below, answer the following questions. (30 pts) CH(9) + S(g) → CS2 (9) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? Show charges C.Given 3.841x1025 molecules of CH4, how many moles is this? D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0°C and 1.25 atm? F.What would be the volume(L)...
6. Given the reaction below, answer the following questions. (30 pts) CH4(g) + S(g) → CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? C.Given 3.841x1025 molecules of CH4, how many moles is this? Show charges D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0°C and 1.25 atm? F.What would be the volume(L)...
CH4(9) + S(g) → CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? C.Given 3.841x1025 molecules of CH4, how many moles is this? Show charges. D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0°C and 1.25 atm? F.What would be the volume(L) of H2S gas (from Part E above) if the temperature was...
answer all questions
ral Chemistry Concept 5 pts Question 1 Balance the chemical equation shown below, Indicate the stoichiometric coefficients for the reaction. Do not leave answer spaces blank if the coefficient is one (1). AIBrg(aq)+ HBr(aq)- Al(s)+ H2(g) The balanced equation will then be used in the following two questions. 5 pts Question 2 Using the balanced chemical equation from the previous question, how many moles of H2(g) will be formed from 6.24 moles of HBr. Your answer will...
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