What are some ways you could lessen your water usage?
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Ответ:
- turning off the water while brushing your teeth.
- turning off the water while washing your hand.
- don’t run the dishwasher or washing machine until it’s full.
- use less electricity.
- take shorter showers
- shower instead of taking a bath
- use a bucket and a sponge to clean your car
- reuse our rain water :)
Ответ:
Note: Since no temperature and pressure conditions are stated, assume STP
2H2(g) + O2(g)
2H2O(g)
At STP, 2(22.4L) 22.4L
2. Dry ice is solid carbon dioxide. What volume of dry ice is produced at STP if 0.50 kg of
dry ice becomes carbon dioxide gas?
CO2 (s)
CO2 (g)
At STP, 44.0 g 22.4 L
3. How many moles of steam are produced at 2.00 atm and 202.0°C by the complete
combustion of 12.50 L of methane gas?
CH4 + 2O2
CO2 + 2H2O
1 mol 2 mol
Note: Since temperature and pressure are stated, STP does not apply
Liter O2 = 40.0 L H2 x 22.4 L O2 = 20 Liters O2
44.8 L H2
Liter CO2 = 500 g CO2 x 22.4 L CO2 = 255 Liters CO2
44.0 g CO2
Given: P = 2.00 atm, T = 202.0 oC + 273 K/oC = 475 K, V CH4 = 12.50 L
First, use given info to find mole of CH4 from PV = nRT
n = PV/RT = 2.00 atm x 12.5 L = 0.641 mol CH4
0.0821 L.atm/mol.K x 475 K
Mol H2O = 0.641 mol CH4 x 2 mol H2O = 1.28 mol H2O
1 mol CH4
4. When nitrogen gas reacts with hydrogen gas, ammonia gas is formed. How many grams
of hydrogen gas are required to react completely with 3.5 L of nitrogen at STP?
N2 + 3H2
2NH3
At STP, 1(22.4L) 6.0g
5. Calculate the mass of water vapor produced when 6.00 L of propane gas undergo
complete combustion at a temperature of 250°C and a pressure of 1.00 atm.
C3H8 + 5O2
3CO2 + 4H2O
1 mol 4(18) g
Note: Since temperature and pressure are stated, STP does not apply
6. A gaseous compound is 30.6% nitrogen and 69.4% oxygen by mass. A 5.25-g sample of
the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C. What is
the molecular formula for the gas?
g H2 = 3.5 L N2 x 6.0 g H2_ = 0.94 g H2
22.4 L N2
Given: V C3H8 =6.00 L, T = 250 oC + 273 K/oC = 523 K, P = 1.00 atm
First, use given info to find mole of C3H8 from PV = nRT
n = PV/RT = 1.00 atm x 6.00 L = 0.1397 mol C3H8
0.0821 L.atm/mol.K x 523 K
Mass H2O = 0.1397 mol C3H8 x 72 g H2O_ = 10.1 g H2O
1mol C3H8
First, find the empirical formula
Element Mass % Number of mole Relative # mol (Divide by smaller # mol)
N 30.6 30.6 g__ = 2.1857 2.1857 = 1
14 g/mol 2.1857
O 69.4 69.4 g___ = 4.3375 4.3375 = 1.98 =2
16 g/mol 2.1857
Hence, empirical formula = NO2
Second, use given data to calculate the molar mass
Molar mass = massRT/PV
Molar mass = 5.25 g x 0.0821 L.atm/mol.K x 269 K = 92.0 g/mol
1.26 atm x 1.00 L
Remember that (empirical formula)x = molar mass
Therefore, (NO2)x = 92.0 Hence, 42x = 92.0; x
Explanation: