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How many liters of hydrogen gas at STP can be produced with 645 grams of baking soda?
To find the volume of hydrogen gas produced, we first need to convert the mass of baking soda (645g) to moles. Then, using the balanced chemical equation for the reaction, we can determine the moles of hydrogen gas produced. Finally, using the ideal gas law at STP, we can convert the moles of hydrogen gas to liters.
How many moles of hydrogen gas are in 5.04 grams in hydrogen gas?
To find the number of moles of hydrogen gas, we first need to convert the mass of hydrogen gas from grams to moles using the molar mass of hydrogen gas (2 g/mol). 5.04 grams of hydrogen gas is equal to 5.04 g / 2 g/mol = 2.52 moles of hydrogen gas.
How do you convert Milliliters of a gas into grams of a gas. For example 475mL O2 to grams?
To convert milliliters of a gas to grams, you need to use the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. To convert 475 mL of O2 to grams, first calculate the number of moles of O2 using the ideal gas law equation. Then, use the molar mass of O2 (32 g/mol) to convert moles to grams: n = PV / RT n = (1 atm) * (0.475 L) / (0.0821 Latm/molK * 298 K) n = 0.0183 mol of O2 m = n * molar mass of O2 m = 0.0183 mol * 32 g/mol m ≈ 0.5856 g
How many grams would 2350 L of O2 gas at STP weigh?
To find the weight of 2350 L of O2 gas at STP, you would first need to calculate the moles of gas using the ideal gas law. Then, use the molar mass of O2 to convert moles to grams. The molar mass of O2 is 32 g/mol, so you would multiply the moles by 32 g/mol to find the weight in grams.
How may grams of calcium carbonate will be needed to form 4.29 liters of carbon dioxide?
To calculate the grams of calcium carbonate needed, you first need to determine the moles of carbon dioxide produced (using the ideal gas law). Then, since 1 mole of CO2 is produced for every mole of CaCO3 consumed, you can convert moles of CO2 to moles of CaCO3. Finally, use the molar mass of CaCO3 to convert moles to grams.
How to convert to moles not at standard temperature and pressure?
Use the ideal gas law, PV=nRT. P= pressure V= volume n= number of moles R= gas law constant T= temperature If you have P, V, R, T then you can solve for "n" to find the number of moles. There are a number of ways and variations that you can go about finding the number of moles, but all would involve the ideal gas law or a similar formula.
How many liters of hydrogen gas at STP can be produced with 645 grams of baking soda?
To find the volume of hydrogen gas produced, we first need to convert the mass of baking soda (645g) to moles. Then, using the balanced chemical equation for the reaction, we can determine the moles of hydrogen gas produced. Finally, using the ideal gas law at STP, we can convert the moles of hydrogen gas to liters.
How many moles of hydrogen gas are in 5.04 grams in hydrogen gas?
To find the number of moles of hydrogen gas, we first need to convert the mass of hydrogen gas from grams to moles using the molar mass of hydrogen gas (2 g/mol). 5.04 grams of hydrogen gas is equal to 5.04 g / 2 g/mol = 2.52 moles of hydrogen gas.
Calculate the mass grams of N2 gas required to occupy a 3.0 mL container at 100 C and 0.914 ATM and explain how you did it?
Use equation n=PV/RT where n is number of moles and R is gas constant. Use R= .8314 L-Atm/mol-K. convert 3 ml to liters(3/1000) and 100C to Kelvin (100+273) and solve for moles. Convert moles to grams. 1 mol of N2 equals 28 grams
How do you convert Milliliters of a gas into grams of a gas. For example 475mL O2 to grams?
To convert milliliters of a gas to grams, you need to use the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. To convert 475 mL of O2 to grams, first calculate the number of moles of O2 using the ideal gas law equation. Then, use the molar mass of O2 (32 g/mol) to convert moles to grams: n = PV / RT n = (1 atm) * (0.475 L) / (0.0821 Latm/molK * 298 K) n = 0.0183 mol of O2 m = n * molar mass of O2 m = 0.0183 mol * 32 g/mol m ≈ 0.5856 g
How many grams would 2350 L of O2 gas at STP weigh?
To find the weight of 2350 L of O2 gas at STP, you would first need to calculate the moles of gas using the ideal gas law. Then, use the molar mass of O2 to convert moles to grams. The molar mass of O2 is 32 g/mol, so you would multiply the moles by 32 g/mol to find the weight in grams.
How may grams of calcium carbonate will be needed to form 4.29 liters of carbon dioxide?
To calculate the grams of calcium carbonate needed, you first need to determine the moles of carbon dioxide produced (using the ideal gas law). Then, since 1 mole of CO2 is produced for every mole of CaCO3 consumed, you can convert moles of CO2 to moles of CaCO3. Finally, use the molar mass of CaCO3 to convert moles to grams.
What mass of chlorine gas will react with 92 grams of sodium?
The balanced chemical equation for the reaction between chlorine gas and sodium is: 2Na + Cl2 -> 2NaCl Using the equation, we can see that 1 mole of chlorine gas (Cl2) reacts with 2 moles of sodium (2Na). To calculate the mass of chlorine gas needed to react with 92 grams of sodium, first convert 92 grams of sodium to moles, then use the mole ratio from the balanced equation to find the moles of chlorine gas needed. Finally, convert the moles of chlorine gas to grams.
How many grams of oxygen gas occupy 2.5 liter container if the pressure is 2.5 ATM and the temperature is 30 C?
To calculate the mass of oxygen gas, use the ideal gas law formula PV = nRT where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. First, convert the temperature to Kelvin (30°C + 273 = 303 K). Then, rearrange the formula to solve for the number of moles (n = PV / RT). Finally, convert moles to grams using the molar mass of oxygen gas (32 g/mol).
Which best represents the number of moles in exactly 84 grams of chlorine (Cl2) gas?
The molar mass of chlorine gas (Cl2) is 70.91 g/mol. To convert grams to moles, you divide the mass (84 g) by the molar mass (70.91 g/mol). So, 84 grams of chlorine gas is equal to approximately 1.18 moles.
How many grams of helium are contained in a 2.0 L balloon at 30 degrees Celsius and at 735 mm Hg?
To find the number of grams of helium in the balloon, you need to use the ideal gas law equation. First, convert the temperature to Kelvin by adding 273 (303 K). Then, convert the pressure to atm (0.966 atm). Now, use the ideal gas law formula: PV = nRT, where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature in Kelvin. Solve for n (moles), which equals 0.08 moles of helium. Finally, calculate the mass using the molar mass of helium (4 g/mol) multiplied by the number of moles (0.08 mol), which equals 0.32 grams of helium.
How many grams of are needed to generate 53.0 of gas if the pressure of is 815 at 21?
To find the number of grams of substance needed, you'll need to consider the ideal gas law, which is PV = nRT. Here are the steps: Calculate the amount of substance (n) using the ideal gas law: n = (PV) / (RT) Convert moles to grams using the molar mass of the substance. Substitute the given values into the equation: P = 815 atm, V = 53.0 L, T = 21 degrees Celsius (294 K), and R = 0.0821 L·atm/(K·mol) for gases. Solve for n and then convert moles to grams.
