<u>Answer:</u> The mass of 
produced will be 8.228 g.
<u>Explanation:</u>
We need to find the mass of carbon dioxide produced when 150 kJ of heat is released.
For the given chemical reaction:
By Stoichiometry of the reaction:
802.3 kJ of energy is released when 1 mole of carbon dioxide is produced.
So, 150 kJ of energy will be release when = 
of carbon dioxide is produced.
To calculate the mass of carbon dioxide, we use the equation:
Moles of carbon dioxide gas = 0.187 mol
Molar mass of carbon dioxide gas = 44 g/mol
Putting values in above equation, we get:
Hence, the mass of produced will be 8.228 g.
The density of the liquid is about 1.85 g/mL.
Density is mass/volume. The volume is given (45.2 mL). The mass must be found by subtracting the tare weight of the graduated cylinder from the total:
95.1 g- 11.4g = 83.7g
Using the mass and volume of the liquid, you can now calculate the density:
d = m/v = 83.7g/45.2 mL = 1.8517699115 g/mL.
Of the original values, the least number of significant figures are 3, so the answer must have a degree of accuracy of 3 significant figures:
1.8517699115 g/mL ≈ 1.85 g/mL.
2NaCl + CaS → Na₂S + CaCl₂
Answer:
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Explanation:
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When 2C2H6 (g) + 7 O2 (g) ⇒ 4CO2 (g) + 6H2O (L) is the balanced equation for this reaction:
So from the equation, 2 mol of C2H6 gives → 4 mol of CO2
So the molar ratio between C2H6 & CO2 is
2 mol C2H6:4 mol CO2 we can make it:
1 mol C2H6: 2 mol Co2
So when we have 5.3 mol of C2H6 how many moles of CO2 then
the moles of CO2 = 5.3 * 2 mol (CO2) / 1 mol (C2H6)
= 10.6 mol
