Molar mass of oxygen is:
M(O)=16 g/mol
Molar mass of carbon is:
M(C)=12 g/mol
Molar mass of carbon dioxide is:
M(CO2)=M(C)+2*M(O)
M(CO2)=12 g/mol+2*16g/mol
M(CO2)=44 g/mol
<span>Molar mass(M) is the mass of 1 mole of the substance (grams per mole of a compound).</span>
1.5M NaOH so we've 1.5 moles of NaOH in 1L of solution
1L = 1000 ml
1.5 moles of NaOH ------------in------------- 1000 ml
0.75 moles of NaOH ----------in---------------x ml
x = 500 ml
<em><u>answer: C</u></em>
Answer:
4.81 moles
Explanation:
The total pressure of the gas = Pressure at which gauge reads zero + pressure read by it.
Pressure at which gauge reads zero = 14.7 psi
Pressure read by the gauge = 988 psi
Total pressure = 14.7 + 988 psi = 1002.7 psi
Also, P (psi) = P (atm) / 14.696
Pressure = 1002.7 / 14.696 = 68.2297 atm
Temperature = 25 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T = (25 + 273.15) K = 298.15 K
Volume = 1.50 L
Using ideal gas equation as:
PV=nRT
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
68.2297 atm × 1.5 L = n × 0.0821 L.atm/K.mol × 298.15 K
⇒n = 4.81 moles
