Answer:
Gas B
Explanation:
diffusion/effusion increases when:
- Temperature increases
- A gas has lower molar mass
- Particles are moving quickly
diffusion/effusion decreases when:
- Temperature decreases
- A gas has higher molar mass
- Particles are moving slowly
Hence: since gas B has the lowest molar mass, it has the highest rate of effusion
I also took the test so I know it is right
Hello!
The concentration of the final solution when a<span> chemistry teacher adds 50.0 mL of 1.50 M H2SO4 solution to 200 mL of water is
0,3 MTo calculate that, you'll need to use the dilution law, where initial and final concentrations are M1 and M2 respectively, and initial and final volumes are V1 and V2, as shown below.
Keep in mind that the final volume is the sum of the 200 mL of water and the 50 mL of H</span>
₂SO₄ that were added by the teacher. ![M2= \frac{M1*V1}{V2}= \frac{1,50 (mol H_2SO_4/L)*50mL}{(50 mL + 200 mL)}=0,3(mol H_2SO_4/L)](https://tex.z-dn.net/?f=M2%3D%20%5Cfrac%7BM1%2AV1%7D%7BV2%7D%3D%20%5Cfrac%7B1%2C50%20%28mol%20H_2SO_4%2FL%29%2A50mL%7D%7B%2850%20mL%20%2B%20200%20mL%29%7D%3D0%2C3%28mol%20H_2SO_4%2FL%29)
Have a nice day!
The difference I think is the fact one has DNA and the other doesn't.
Answer:
by using ideal gas law
Explanation:
ideal gas law:
PV=nRT
where:
P is pressure measured in Pascal (pa)
V is volume measured in letters (L)
n is number of moles
R is ideal gas constant
T is temperature measured in Kelvin (K)
by applying the given:
P(initial) V(initial)=nRT(initial)
P(final) V(final)=nRT(final)
nR is constant in both equations since same gas
then,
P(initial) V(initial) / T(initial) = P(final) V(final) / T(final)
then by crossing multiply both equations
V (final)= { (P(initial) V(initial) / T(initial)) T(final) } /P (final)
P(initial)=P(final)= 1 atm = 101325 pa
V(initial)= 6 L
T(initial) = 28°c = 28+273 kelvin
T(final) = 39°c = 39+273 kelvin
by substitution
V(final) = 6.21926 L