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For this problem you have to use PV=nRT.
In order to get anywhere with the question, you have to isolate the V (volume) and get it alone. To do that, you have to divide each side by P (pressure). When you do that, your new formula to work with is:
V = nRT / P
(the P cancelled out on the other side, which left you with V)
Unfortunately, you weren't given the number of moles in the problem. Instead, they made it a bit more challenging by giving you the number of grams, which can be converted to give you your number of moles:
42 g / 1 ( 1 mole / 28.01 g) = 1.5 moles of CO
Now, you have all the information that you need in order to answer the question. All you have to do now is plug in, but make sure that you know where everything goes:
n (moles) = 1.5 moles
R = .0821 L atm / mole K <-----that one looks weird, but that's all required for R
T (temp) = 273 K <----that's your standard temp *must be in Kelvin!!!! ALWAYS!!
P (pressure) = 1 atm <----standard pressure for P *must be in atm!! ALWAYS!!
Your equation should now look like this:
V= (1.5 moles x .0821 Latm/ moleK x 273 K) / (1 atm) =
34 L CO
And then you get your answer!
What else can I help you with?
What is the volume in milliliters occupied by 89.2g CO2(g) at 37oC and 737 mmHg?
To find the volume of a gas using the ideal gas law formula PV = nRT, we need to know the molar mass of CO2 (44.01 g/mol) and convert grams to moles. Then we can rearrange the formula to solve for V (volume) using P (pressure), n (moles), R (gas constant), and T (temperature). After plugging in the values (P = 737 mmHg, T = 37°C + 273 = 310 K), we can calculate the volume occupied by 89.2g of CO2 gas.
How can the student make a quantitative observation of the CO2 collected in the balloons?
The student can measure the volume of CO2 collected in each balloon using a graduated cylinder or syringe to calculate the total volume of gas. They could then compare the mass of the balloons before and after the experiment to determine the mass of CO2 collected. Finally, they could use a color-changing pH indicator to analyze the acidity of the collected gas, indicating the presence of CO2.
What volume does 22g of CO2 at STP occupy?
This depends on the temperature and the pressure. At standard temperature and pressure 1 mole will occupy 22.4 L, so multiply... 22.4 x 2.22 = 48.728 L at STP.
How many grams does 3 moles of CO2 weigh?
Atomic mass of C = 14g/mol Atomic mass of O = 16g/mol Molecular mass of CO2 = 12 + 2(16) = 44g/mol mass = number of moles x molecular mass mass = 3 mol x 44g/mol = 132g
What is the volume of a sample of co2 at stp that has a volume of 75.0 ml at 30.0c and 91 kpa?
To calculate the volume of CO2 at STP (Standard Temperature and Pressure), you can use the ideal gas law equation: PV = nRT. First, find the number of moles of CO2 using the ideal gas law equation. Then, use the molar volume of a gas at STP (22.4 L/mol) to find the volume at STP.
What is the volume in milliliters occupied by 89.2g CO2(g) at 37oC and 737 mmHg?
To find the volume of a gas using the ideal gas law formula PV = nRT, we need to know the molar mass of CO2 (44.01 g/mol) and convert grams to moles. Then we can rearrange the formula to solve for V (volume) using P (pressure), n (moles), R (gas constant), and T (temperature). After plugging in the values (P = 737 mmHg, T = 37°C + 273 = 310 K), we can calculate the volume occupied by 89.2g of CO2 gas.
What is the meaning of percent of carbon dioxide in auto emissions?
Auto emits carbon monoxide(CO), carbon dioxide(CO2) and some other gases and particles which pollute the environment. the amount of CO2 compared to total amount of emission in percentage is called as percent of carbon dioxide in auto emissions. %CO2=(Volume of CO2 emitted/Total volume of emission)*100
What is the volume occupied by 20.4 liters of co2 at 1200 torr when it is STP?
To find the volume occupied by 20.4 liters of CO2 at STP (Standard Temperature and Pressure, defined as 0°C and 1 atm), we can use the ideal gas law and the concept of proportionality. At STP, 1 mole of gas occupies 22.4 liters, and 1200 torr is approximately 1.58 atm. Using the combined gas law, we can calculate the volume at STP: [ V_{STP} = V_{initial} \times \frac{P_{initial}}{P_{STP}} \times \frac{T_{STP}}{T_{initial}} ] Substituting the known values, the volume at STP will be approximately 12.9 liters.
How can the student make a quantitative observation of the CO2 collected in the balloons?
The student can measure the volume of CO2 collected in each balloon using a graduated cylinder or syringe to calculate the total volume of gas. They could then compare the mass of the balloons before and after the experiment to determine the mass of CO2 collected. Finally, they could use a color-changing pH indicator to analyze the acidity of the collected gas, indicating the presence of CO2.
How do you figure ppm of CO2 in the air?
To calculate the parts per million (ppm) of CO2 in the air, you would measure the concentration of CO2 in the air using a CO2 sensor or monitor, and then divide that by the total volume of the air sample. This would give you the ppm of CO2 in the air sample. Common methods include using infrared gas analyzers or chemical absorbents.
Why dry ice CO2 floats?
CO2 floats because its density is less then water. Anything will float if its density is less then water. That is; when a certain volume of CO2 (or anything else) weighs less then the same volume of water.
What volume does 22g of CO2 at STP occupy?
This depends on the temperature and the pressure. At standard temperature and pressure 1 mole will occupy 22.4 L, so multiply... 22.4 x 2.22 = 48.728 L at STP.
How much co2 in soda stream bottle?
The amount of CO2 in a SodaStream bottle varies depending on the carbonation level desired. Typically, a standard SodaStream CO2 cylinder can carbonate up to 60 liters of water, infusing it with approximately 0.5 to 0.9 grams of CO2 per liter, depending on the user's preference for fizziness. In terms of total CO2 volume, this equates to around 30 to 54 grams of CO2 per cylinder.
What volume of CO2 forms from 5.25 grams of CaCo3 at 103killipascals and 25 degrees Celsius?
To calculate the volume of CO2 formed, first determine the moles of CaCO3 using its molar mass. Then, calculate the moles of CO2 produced assuming all the CaCO3 is converted to CO2. Finally, use the ideal gas law (PV = nRT) to find the volume of CO2 at 103 kPa and 25°C. Be sure to convert Celsius to Kelvin (273 + 25).
How many grams does 3 moles of CO2 weigh?
Atomic mass of C = 14g/mol Atomic mass of O = 16g/mol Molecular mass of CO2 = 12 + 2(16) = 44g/mol mass = number of moles x molecular mass mass = 3 mol x 44g/mol = 132g
What is the volume of a sample of co2 at stp that has a volume of 75.0 ml at 30.0c and 91 kpa?
To calculate the volume of CO2 at STP (Standard Temperature and Pressure), you can use the ideal gas law equation: PV = nRT. First, find the number of moles of CO2 using the ideal gas law equation. Then, use the molar volume of a gas at STP (22.4 L/mol) to find the volume at STP.
What is the calculated molar volume of the dry CO2?
The molar volume of dry carbon dioxide (CO2) at standard temperature and pressure (STP) is approximately 22.4 liters per mole.
