Methane gas and chlorine gas react to form hydrogen chloride gas and carbon tetrachloride gas. What volume of hydrogen chloride would be produced by this reaction if 3.16 L of chlorine were consumed at STP.
Be sure your answer has the correct number of significant digits.
Answer: Thus volume of carbon tetrachloride that would be produced is 0.788 L
Explanation:
According to ideal gas equation:

P = pressure of gas = 1 atm (at STP)
V = Volume of gas = 3.16 L
n = number of moles = ?
R = gas constant =
T =temperature =



According to stoichiometry:
4 moles of chlorine produces = 1 mole of carbon tetrachloride
Thus 0.141 moles of methane produces =
moles of carbon tetrachloride
volume of carbon tetrachloride =
Thus volume of carbon tetrachloride that would be produced is 0.788 L
It forms Carbon monoxide.
CO2 +O2⇒ CO
(Sorry not balanced)
Answer:
4.15×10⁻²¹ moles of Sn
Explanation:
This question can be solved by a simple rule of three.
We know that 1 mol contains 6.02×10²³ particles.
In this case, our particles are the atoms, so:
6.02×10²³ atoms / 1 mol . 2500 atoms = 4.15×10⁻²¹ moles.
The knowledge of mol can be applied for everything:
A mol of molecules
A mol of atoms
A mol of a compound
2NBr₃ + 3NaOH = N₂ + 3HOBr + 3NaBr
40 mol 48 mol
NBr₃:NaOH = 2:3
40:48 = 2:2.4 = 2.5:3
NBr₃ is the excess reactant