CHEMISTRY HELP! I would appreciate it if someone could walk me through it. I am

Question

CHEMISTRY HELP! I would appreciate it if someone could walk me through it. I am trying to do Part B, C, and D.

When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is

CH4(g)+O2(g)?CO2(g)+H2O(g)

This type of reaction is referred to as a complete combustion reaction.

Part A

What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H2O, respectively.

Express your answer as four integers, separated by commas (e.g., 1,2,3,4).

1,2,1,2

Part B.

What mass of carbon dioxide is produced from the complete combustion of 9.00

Explanation / Answer

(1) CH4(g) + 2 O2(g) => CO2(g) + 2 H2O(g)

Coefficients are 1,2,1,2

(2) Moles of CH4 = mass/molar mass of CH4

= 9.00 x 10^(-3)/16.04 = 5.611 x 10^(-4) mol

Moles of CO2 = moles of CH4 = 5.611 x 10^(-4) mol

Mass of CO2 = moles x molar mass of CO2

= 5.611 x 10^(-4) mol x 44.01

= 0.0247 g = 2.47 x 10^(-2) g

(3) Moles of H2O = 2 x moles of CH4

= 2 x 5.611 x 10^(-4) = 1.122 x 10^(-3) mol

Mass of H2O = moles x molar mass of H2O

= 1.122 x 10^(-3) x 18.02

= 0.0202 g = 2.02 x 10^(-2) g

(4) Moles of O2 = 2 x moles of CH4

= 2 x 5.611 x 10^(-4) = 1.122 x 10^(-3) mol

Mass of O2 = moles x molar mass of O2

= 1.122 x 10^(-3) x 32.00

= 0.0359 g = 3.59 x 10^(-2) g

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