Answer: 4.90
Explanation: The molal freezing point constant of C6H6 is 4.90 and its melting point is 5.51∘C. A solution of 0.816 g of a compound A dissolved in 7.5 g of benzene freezes at 1.59∘C. Calculate molecular weight of compound A
E. 0.42 meters / second
Since you are finding the average speed, you don't need to factor in all the stops Mary makes on her way to her final destination. Add the total distance she walked ( 80 + 125 + 45 ) and divide it by the amount of time IN SECONDS that it took for her to do this. Since the time given is in minutes, simply multiply the number of minutes ( 10 ) by 60 ( the amount of seconds in a minute ). Then divide the total number of meters walked by the total amount of seconds it took to walk, and you will get your average speed.
( Also, this is a Physics question, not Chemistry :D )
If the mass of both the reactants is 10kg then the mass of the products also equals 10kg.
It is due to the law of conservation of mass.
Mass can neither be created nor be destroyed.
Explanation:
Reaction equation:
CO + 2H₂ → CH₃OH
All the species are in gaseous state and the equation is balanced.
Change in pressure only affects equilibrium involving a gas or gases.
Based on Le Chatelier's principle, an increase in pressure will shift the position of equilibrium to the side having smaller volume or number of moles and vice versa.
CO + 2H₂ → CH₃OH
3moles of gases 1 mole of gas
An increase in pressure favors the forward reaction. A decrease in pressure will favor the backward step.
Answer:
1.17 L of H₂
Explanation:
We'll begin by calculating the number of mole in 2.3 g of Mg. This can be obtained as follow:
Mass of Mg = 2.3 g
Molar mass of Mg = 24 g/mol
Mole of Mg =?
Mole = mass /molar mass
Mole of Mg = 2.3 / 24
Mole of Mg = 0.096 mole
Next, we shall determine the number of mole of H₂ produced by the reaction of 2.3 g (i.e 0.096 mole) of Mg. This can be obtained as follow:
Mg + 2HCl —> MgCl₂ + H₂
From the balanced equation above,
1 mole of Mg reacted to 1 mole of H₂.
Therefore, 0.096 mole of Mg will also react to produce 0.096 mole of H₂.
Finally, we shall determine volume of H₂ produced from the reaction. This can be obtained as follow:
Number of mole (n) of H₂ = 0.096 mole
Pressure (P) = 2 atm
Temperature (T) = 298 K
Gas constant (R) = 0.0821 atm.L/Kmol
Volume (V) of H₂ =?
PV = nRT
2 × V = 0.096 × 0.0821 × 298
Divide both side by 2
V = (0.096 × 0.0821 × 298) /2
V = 1.17 L
Therefore, 1.17 L of H₂ were obtained from the reaction.