How many moles of water are produced from 19.2g of B2H6
Answers
Answer:
Balance the following chemical reactions:
a. 2 CO + O2 2 CO2
b. 2 KNO3 2 KNO2 + O2
c. 2 O3 3 O2
d. NH4NO3 N2O + 2 H2O
e. 4 CH3NH2 + 9 O2 4 CO2 + 10 H2O + 2 N2
f. Cr(OH)3 + 3 HClO4 Cr(ClO4)3 + 3 H2O
Write the balanced chemical equations of each reaction:
a. Calcium carbide (CaC2) reacts with water to form calcium hydroxide (Ca(OH)2) and acetylene gas (C2H2).
CaC2 + 2 H2O C2H2 + Ca(OH)2
b. When potassium chlorate (KClO3) is heated, it decomposes to form KCl and oxygen gas (O2).
2 KClO3 2 KCl + 3 O2
c. C6H6 combusts in air.
2 C6H6 + 15 O2 12 CO2 + 6 H2O
d. C5H12O combusts in air.
2 C5H12O + 15 O2 10 CO2 + 12 H2O
Given the following reaction: Na2S2O3 + AgBr NaBr + Na3[Ag(S2O3)2]
a. How many moles of Na2S2O3 are needed to react completely with 42.7 g of AgBr? 0.455 mol Na2S2O3
b. What is the mass of NaBr that will be produced from 42.7 g of AgBr? 23.4 g NaBr
From the reaction: B2H6 + O2 HBO2 + H2O
a. What mass of O2 will be needed to burn 36.1 g of B2H6? 125 g O2
b. How many moles of water are produced from 19.2 g of B2H6? 1.39 mol H2O
Calculate the mass (in kg) of water produced from the combustion of 1.0 gallon (3.8 L) of gasoline (C8H18). The density of gasoline is 0.79 g/mL.
Answer:
Balance the following chemical reactions:
a. 2 CO + O2 2 CO2
b. 2 KNO3 2 KNO2 + O2
c. 2 O3 3 O2
d. NH4NO3 N2O + 2 H2O
e. 4 CH3NH2 + 9 O2 4 CO2 + 10 H2O + 2 N2
f. Cr(OH)3 + 3 HClO4 Cr(ClO4)3 + 3 H2O
Write the balanced chemical equations of each reaction:
a. Calcium carbide (CaC2) reacts with water to form calcium hydroxide (Ca(OH)2) and acetylene gas (C2H2).
CaC2 + 2 H2O C2H2 + Ca(OH)2
b. When potassium chlorate (KClO3) is heated, it decomposes to form KCl and oxygen gas (O2).
2 KClO3 2 KCl + 3 O2
c. C6H6 combusts in air.
2 C6H6 + 15 O2 12 CO2 + 6 H2O
d. C5H12O combusts in air.
2 C5H12O + 15 O2 10 CO2 + 12 H2O
Given the following reaction: Na2S2O3 + AgBr NaBr + Na3[Ag(S2O3)2]
a. How many moles of Na2S2O3 are needed to react completely with 42.7 g of AgBr? 0.455 mol Na2S2O3
b. What is the mass of NaBr that will be produced from 42.7 g of AgBr? 23.4 g NaBr
From the reaction: B2H6 + O2 HBO2 + H2O
a. What mass of O2 will be needed to burn 36.1 g of B2H6? 125 g O2
b. How many moles of water are produced from 19.2 g of B2H6? 1.39 mol H2O
Calculate the mass (in kg) of water produced from the combustion of 1.0 gallon (3.8 L) of gasoline (C8H18). The density of gasoline is 0.79 g/mL.