The mass of a sample of alcohol is found to be = m = 367 g
Hence, it is found out that by raising the temperature of the given product, the mass of alcohol would be 367 g.
Explanation:
The Energy of the sample given is q = 4780
We are required to find the mass of alcohol m = ?
Given that,
The specific heat given is represented by = c = 2.4 J/gC
The temperature given is ΔT = 5.43° C
The mass of sample of alcohol can be found as follows,
The formula is c =
We can drive value of m bu shifting m on the left hand side,
m =
mass of alcohol (m) =
m = 367 g
Therefore, The mass of the given sample of alcohol is
m = 367g
It requires 4780 J of heat to raise the temperature by 5.43 C in the process which yields a mass of 367 g of alcohol.
Answer:
The final volume of the sample of gas = 0.000151
Explanation:
Initial volume = 200 ml = 0.0002
Initial temperature = 296 K
Initial pressure = 101.3 K pa
Final temperature = 336 K
Final pressure = K pa
Relation between P , V & T is given by
Put all the values in the above equation we get
= 0.000151
This is the final volume of the sample of gas.
Explanation:
The given reaction equation will be as follows.
Now, number of atoms on reactant side are as follows.
Number of atoms on product side are as follows.
Therefore, this equation is balanced since atoms on both reactant and product sides are equal.
Thus, we can conclude that there is one sulfur atom in the products.