Are you doing a research on C5 burning?I am Zy from China.
To make it easier, assume that we have a total of 100 g of a compound. Hence, we have 58.80g of xenon, 7.166g of oxygen, and 34.04g of fluorine.
Know we will convert each of these masses to moles by using the atomic masses:
58.8/131.3 = 0.45 mole of Xe
7.166/16 = 0.45 mole of O
34.04/19 = 1.79 mole of F
Now, we will divide all the mole numbers by the smallest among them and get the number of atoms in the compound:
Xe = 0.45/0.45 = 1
O = 045/0.45 = 1
F = 1.79/0.45 = 3.98 = 4
So, the empirical formula of the compound XeOF₄
That would be 222.0 mm to 4 sig figs
Answer:
We need 4.06 J to heat of 406.0 mg of cyclohexane
Explanation:
Step 1: Data given
Mass of cyclohexane = 406.0 mg = 0.406 grams
The initial temperature = 33.5 °C
The final temperature = 38.9 °C
The specific heat of cyclohexane = 1.85 J/g*K
Step 2: Calculate the energy required to heat
Q = m*c*ΔT
⇒ with m = the mass of cyclohexane = 0.406 grams
⇒ with c = the specific heat of cyclohexane = 1.85J/g*K
⇒ with ΔT = The change of temperature = T2 - T1 = 38.9 - 33.5 = 5.4
Q = 0.406 g * 1.85J/g*K * 5.40
Q = 4.06 J
We need 4.06 J to heat of 406.0 mg of cyclohexane
Molar mass Na2SO4 = <span>142.04 g/mol
142.04 g -------------- 6.02x10</span>²³ atoms
?? g ------------------ 7.4x10²³ atoms
142.04 x ( 7.4x10²³) / 6.02x10²³
=> 174.60 g