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3 years ago

This calculation shows that burning _ grams of methane (takes in/gives off) _ energy

1 answer:

8 0

The question lacks some details in order to be answered. Nevertheless, let's just give some examples.

Given that you are to burn 10 kg of methane (CH4) from 0 to 20°C. The specific heat capacity of methane is 4.475 kJ/kg-K.

H = mCpT
H = (10kg)( 4.475 kJ/kg-K)(20-0)
H = 895.00 kJ

Because of the positive value of enthalpy, methane takes in heat.

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In a chemical reaction, sulfur (S8) combines with copper to give a pure compound. If you start with 1.000 g of sulfur (S8) and o

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Answer: The empirical formula for the given compound is $Cu_2S$

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We are given:

Mass of pure compound containing copper and sulfur = 4.963 g

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To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Copper = $\frac{\text{Given mass of Copper}}{\text{Molar mass of Copper}}=\frac{3.963g}{63.55g/mole}=0.0624moles$

Moles of Sulfur = $\frac{\text{Given mass of Sulfur}}{\text{Molar mass of Sulfur}}=\frac{1.000g}{32g/mole}=0.0312moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0312 moles.

For Copper = $\frac{0.0624}{0.0312}=2$

For Sulfur = $\frac{0.0312}{0.0312}=1$

Step 3: Taking the mole ratio as their subscripts.

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This calculation shows that burning ___ grams of methane (takes in/gives off) ___ energy

This calculation shows that burning _ grams of methane (takes in/gives off) _ energy