chemgirl26 chemgirl26

28-10-2022
Chemistry

Answered

5. The alcohol is “gasohol” burns according to the following equation: 2CH3OH +3O2 —> 2CO2 + 4H2O

If 75.50 g of CH3OH is burned in the presence of 65.50 g of O2, calculate the theoretical yield of CO2 in grams

If 40.1 g of CO2 were collected in the previous problem, calculate the percent yield

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Other Questions

3. The alcohol is “gasohol” burns according to the following equation: 2CH3OH +3O2 —> 2CO2 + 4H2O how many grams of O2 are produced when 120.0 g of CH3OH i

1. The alcohol is “gasohol” burns according to the following equation: 2CH3OH +3O2 —> 2CO2 + 4H2O how many grams of CO2 are produced when 120.0 g of CH3OH i

2. The alcohol is “gasohol” burns according to the following equation: 2CH3OH +3O2 —> 2CO2 + 4H2O how many grams of H2O are produced when 120.0 g of CH3OH

CH3CH2CH2CO2H(l)+CH2CH3OH(l)H+⟶CH3CH2CH2CO2CH2CH3(l)+H2O(l) A chemist ran the reaction and obtained 5.75 g of ethyl butyrate. What was the percent yield?

What is the empirical formula of a compound containing C, H, and O if combustion of 1.23 g of the compound yields 2.46 g CO2 and 1.01 g H₂O?

Consider the reaction CH4 + 20₂ = CO₂ + 2H₂O. If 8.01 grams of CH4 are burned in excess O2, 445 kilojoules of heat are evolved. Heats of formation: CH4 = -74.8

Calculate mass of (8.0*10^ ^ 22) molecules of HL

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