Suppose that brown coal from a certain mine is 80.0% carbon by mass and the rema

Question

Suppose that brown coal from a certain mine is 80.0% carbon by mass and the remainder is inert material. The coal is removed at a rate of 5000. kg/hour. The coal is burned to produce electricity. How many kg and moles CO_2, a greenhouse gas, are produced from the coal that is mined during one 8 hour shift? A compound X contains 63.3% manganese and 36.7% oxygen by mass. When X is heated, oxygen gas is evolved and a new compound Y is containing 72.0% manganese and 28.0% oxygen formed. What are the empirical formulas for compounds X and Y? Write a balanced equation for the conversion of X to Y. A quantity of 25.0 mL of a solution containing both Fe^2+ and Fe^3+ ions is titrated with 23.0 mL of 0.0200 M KMnO_4 in dilute acidic solution. As a result, all of the Fe^2+ ions arc converted to Fe^3+ ions. Next, the solution is treated with zinc metal to convert all of the Fe^3+ ions to Fe^2+ ions. Finally, the solution containing only Fe^2+ ions requires 40.0 mL. If the same KMnO_4 solution. Calculate the molar concentration of the Fe^2+ and Fe^3+ ions in the original solution. The net ionic equation is: MnO_4^- + 5Fe^2+ + 8H^+ rightarrow Mn^2+ + 5Fe^3+ + 4H_2O

Explanation / Answer

C + O2 ----> CO2

According to the balanced equation 12 gm C burn to produce 44gm of CO2.

In one hour 5000Kg coal is burnt. So, in 8 hour 8*5000kg = 40,000kg coal is burnt.

amount of carbon in 40,000kg carbon = 40,000* 80/100 = 32,000kg

Mass of CO2 produced = 32,000kg* (44/12) = 117333.33 kg

Moles of CO2 produded = 117333.33*10^3/44gm/mol = 2666.67 *10^3 moles

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