The number of hydrogen atoms that are in 4.40 mol of ammonium sulfide is 2.12 x10^25 atoms
calculation
find the number of moles of Hydrogen in ammonium sulfide (NH4)2S
that is 4.40 x number of hydrogen atoms in (NH4)2S ( 4x2= 8 atoms)
moles is therefore= 4.40 x8= 35.2 moles
by use of Avogadro's law constant
that is 1mole = 6.02 x10^23 atoms
35.2 moles=?
by cross multiplication
{35.2 moles x 6.02 x10^23} /1 mole = 2.12 x10^25 atoms
Answer:
0.1 mole of CH₄
Explanation:
From the question given above, the following data were obtained:
Volume of CH₄ = 2.24 L
Number of mole of CH₄ =?
The number of mole of CH₄ can be obtained as follow:
Recall:
1 mole of a gas occupy 22.4 L at stp. This implies that 1 mole of CH₄ occupies 22.4 L at stp.
22.4 L = 1 mole of CH₄
Therefore,
2.24 L = 2.24 × 1 mole of CH₄ / 22.4
2.24 L = 0.1 mole of CH₄.
I haven't got the answer but I'm probably sure that u can actually look up that answer hoped it help
Explanation:
1. Spontaneous as written at all temperatures
C. When ΔH is negative and ΔS is positive, the sign of ΔG will always be negative, and the reaction will be spontaneous at all temperatures.
2. Spontaneous in reverse at all temperatures
A. When ΔH is positive and ΔS is negative, the sign of ΔG will always be positive, and the reaction can never be spontaneous.
3. Spontaneous as written above a certain temperature
B. ΔH is positive and ΔS is positive - an endothermic reaction (positive ΔH) that also displays an increase in entropy (positive ΔS). It is the entropy term that favors the reaction. Therefore, as the temperature increases, the TΔS term in the Gibbs free energy equation will begin to predominate and ΔG will become negative.
4. Spontaneous as written below a certain temperature
D. ΔH negative and ΔS is negative - When the reaction is exothermic (negative ΔH) but undergoes a decrease in entropy (negative ΔS), it is the enthalpy term which favors the reaction. In this case, a spontaneous reaction is dependent upon the TΔS term being small relative to the ΔH term, so that ΔG is negative. The freezing of water is an example of this type of process. It is spontaneous only at a relatively low temperature.
