Given: 8CO + 17H2 → C8H18 + 8H2O In this chemical reaction, how many grams of H2 will react completely with 6.50 moles of CO? Ex
2 answers:
Answer:- 27.6 grams of hydrogen are required.
Solution:- The given balanced equation is:
From balanced equation, there is 8:17 mol ratio between CO and means 17 moles of hydrogen are required to react completely with 8 moles of CO.
Let's calculate the number of moles of hydrogen required to react completely with 6.50 moles of CO and convert to grams on multiplying by molar mass of hydrogen as:
=
So, 27.6 grams of hydrogen are required to react completely with 6.50 moles of CO.
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Answer : The new pressure if the volume changes to 560.0 mL is, 280 mmHg
Explanation :
According to the Boyle's, law, the pressure of the gas is inversely proportional to the volume of gas at constant temperature and moles of gas.
or,
where,
= initial pressure = 560.00 mmHg
= final pressure = ?
= initial volume = 280 mL
= final volume = 560.0 mL
Now put all the given values in the above formula, we get:
Therefore, the new pressure if the volume changes to 560.0 mL is, 280 mmHg
Answer:
Explanation: A yellow precipitate o lead iodide is formed. see equation of reaction below: →
Th PbI2 is the insoluble yellow precipitate