A sample of helium gas has a volume of 0.180L, a pressure of 0.800a and a temperature of 29 C. What is the new temp or gas of volume of 90mL and pressure of 3.20 atm

The new temperature of the gas is 604K

Explanation:

Assuming standard temperature and pressure, to calculate the temperature of the gas we use the general gas equation;

Step 1 :write the general gas equation

P1V1/ T1 = P2V2/T2

Step 2: Write out the values, covert the necessary values to the standard values.

P1 = 0.800atm.

V1 = 0.180L

T1 = 29°C = 273 + 29 = 302K

P2 , 3.20atm

V2 = 90mL = 90 * 10^-3L = 0.09L

Step 3: Solve for T2

The new temperature T2 of the gas is:

T2 = P2V2T1/ P1V1

T2 = 3.20 * 0.09 * 302 / 0.800 * 0.180

T2 = 86.976 / 0.144

T2 = 604K

The new temperature is of the gas is 604K.

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

answer: i have one answer

acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (h+) ions

explanation:

hope this and sorry i could only come up with one answer!