[Answer] The value of ΔH° for the reaction below is +128.1 kJ:CH3OH(l) → CO(g) + 2H2(g)How many kJ of heat are consumed when 5.10 g of CO(g) is formed as shown in the equation?

Answer: exothermic released

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The value of ΔH° for the reaction below is +128.1 kJ:CH3OH(l) → CO(g) + 2H2(g)How many kJ of heat are consumed when 5.10 g of CO(g) is formed as shown in the equation? The value of ΔH° for the reaction below is +128.1 kJ: CH3OH (l) → CO (g) + 2H2 (g) How many kJ of heat are consumed when 5.10 g of CO (g) is formed as shown in the equation ? The value of ΔH ° for the reaction below is +128.1 kJ: CH3OH ( l ) → CO ( g ) + 2H2 ( g ) How many kJ of heat are consumed when 15.5 g of CH3OH ( l ) decomposes as shown in the equation ? We are asked to calculate the kJ of heat that are consumed when 5.10 g of CO ( g ) is formed . The reaction is already balanced: CH 3 OH ( l ) → CO ( g ) + 2 H 2 ( g ) CO ( g ) has a coefficient of only 1. This means that + 128.1 kJ is consumed per 1 mole of CO . We are given the mass so we still need to … The value of ΔH ° for the reaction below is +128.1 kJ: CH3OH ( l ) → CO ( g ) + 2H2 ( g ) How many kJ of heat are consumed when 15.5 g of CH3OH ( l ) decomposes as shown in the equation ? We are asked to calculate the kJ of heat that are consumed when 5.10 g of CO ( g ) is formed . Sun Feb 14 2016 · The value of ΔH ° for the reaction below is +128.1 kJ: CH3OH ( l ) → CO ( g ) + 2H2 ( g )? How many kJ of heat are consumed...

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