A stove needs gas to burn (I only have one off the top of my head, sorry :/)
Answer:
1) They are the same line so they match equally bc they are measuring the same thing just one is more specific than the other
2) Sonar measures all depths at every possible point and maps it including all the gaps in between the 5cm apart the ocean floor is. The difference between the points could be a cliff or a smooth decline.
Answer:
<h3>1. B</h3><h3>2. A</h3><h3>3. B</h3><h3>4. B</h3><h3>5. C</h3><h3>I HOPE IT HELPS :) 100% sureness</h3>
Based on the data given, the molar mass of the gas is 165.5 g/mol while the molecular weight of the gas is 165.5 amu
<h3>How can molar mass of a gas be obtained from density, temperature and pressure?</h3>
The molar mass of a gas can be obtained from density, temperature and pressure using the formula below:
- molar mass = density × molar gas constant × temperature/pressure
Molar gas constant, R = R = 0.082 L.atm/mol/K.
Temperature = 150 °C = 423 K
Pressure = 785 torr = 1.033 atm
density = 4.93 g/L
molar mass of gas = 4.93 × 0.082 × 423/1.033
molar mass of gas = 165.5 g/mol
Then, molecular weight of the gas = 165.5 amu
Therefore, the molar mass of the gas is 165.5 g/mol while the molecular weight of the gas is 165.5 amu
Learn more about molar mass of a gas at: brainly.com/question/26215522
Answer:
y1 = 0.3162
y2 = 0.6838
Explanation:
ok let us begin,
first we would be defining the parameters;
at 25°C;
1-propanol P1° = 20.90 Torr
2-propanol P2° = 45.2 Torr
From Raoults law:
P(1-propanol) = P⁰ × X(1-propanol)
P(1-propanol) = 20.9 torr × 0.45 = 9.405
P(1-propanol) = 9.405 torr
Also P(2-propanol) = P⁰ × X(2-propanol)
P(2-propanol) = 45.2 torr × 0.45
P(2-propanol) = 20.34 torr
but the total pressure = sum of individual pressures
total pressure = 9.405 + 20.34
total pressure = 29.745 torr
given that y1 and y2 represent the mole fraction of each in the vapor phase
y1 = P1 / total pressure
y1 = 9.405/29.745
y1 = 0.3162
Since y1 + y2 = 1
y2 = 1 - y1
∴ y2 = 1 - 0.3162
y2 = 0.6838
cheers, i hope this helps.
