In the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide water and energy. How many moles of CO2 are formed fr

Question

In the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide water and energy. How many moles of CO2 are formed from the reaction with 1.20 moles of C2H2?

Given the following equation
2C2H2(g) + 502(g) = 4CO2(g) + 2H2O(g)

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Đan Thu 5 years 2021-07-29T17:49:49+00:00 1 Answers 63 views 0

Answers ( )

  1. minhkhang
    0
    2021-07-29T17:50:54+00:00
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    Answer: 2.40 moles of CO_2 will be formed in the reaction.

    Explanation:

    Given values:

    Moles of C_2H_2 = 1.20 moles

    The given chemical equation follows:

    2C_2H_2+5O_2\rightarrow 4CO_2+2H_2O

    By the stoichioemetry of the reaction:

    If 2 moles of C_2H_2 produces 4 moles of carbon dioxide

    Then, 1.20 moles of C_2H_2 wil produce = \frac{4}{2}\times 1.20=2.40mol of carbon dioxide

    Hence, 2.40 moles of CO_2 will be formed in the reaction.

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