Answer:
mass of hydrogen collected is 0.016 gram
Explanation:
Given values:
For calculating mass we have to find the number of moles first
Ideal gas equation PV =nRT
Volume= 195 ml
Pressure: 753 torr =0.99 atm
Temperature: 25+273= 298 Kelvin
Ideal gas constant R= 0.0821 Latm/molK
Number of moles n= ?
So n= PV/RT
Adding the values
n= = (753 torr)(1 atm/760 torr)(195 mL)(1 L/1000 mL)/(0.0821 L·atm/mol·K)(273 K)
n = 0.007897 moles of H₂
Now mass of hydrogen collected = number of moles x Molar mass of H₂
= 0.007897 x 2
= 0.0157 g H₂
Now mass of hydrogen collected is 0.016 gram (rounding the amount)
0.50 moles of oxygen gas will react.
Balanced chemical eqation for reaction of calcium with oxygen:
2Ca + O₂ → 2CaO
n(Ca) = 1.0 mol; amount of calcium
From balanced chemical reaction, we can see that 2 moles of calcium reacts with one mole of oxygen gas. Ratio of moles is 2 : 1.
n(Ca) : n(O₂) = 2 : 1; ratio of the amount of substance of calcium and oxygen gas
n(O₂) = n(Ca) / 2; two times less amount of oxygen than calcium
n(O₂) = 1.0 mol / 2
n(O₂) = 0.5 mol; amount of oxygen gas needed for this chemical reaction.
More about stoichiometry: brainly.com/question/16060223
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Answer:
1. kmol of methanol= 3.12 Kmol
2. kmol of water= 5.55 Kmol
3. Liters of methanol= 126.4 L
4. L of water= 100 L
Explanation:
1. kmol of methanol?
32.04 kg methanol ______________ 1 kmol of methanol
100 kg of methanol_______________ X= 3.12 kmol ofmethanol
2. kmol of water?
18.01 kg water ______________ 1 kmol of wáter
100 kg of wáter_______________ X= 5.55 kmol of water
3. Liters of methanol?
0.791 kg methanol _______________________1.00 L of methanol
100kg methanol _______________________x= 126.4 L of methanol
4. L of water?
1kg water _______________________1.00 L of water
100kg water _______________________x= 100 L of water
Answer:The molar mass of a compound cab be find by adding up all the molar mass of the element present in the compound... Check the image for more clarification
Explanation: