calculate the pressure inside a 20 L airbag that inflates with 3 moles of N2 at 20 C
calculate the pressure inside a 20 L airbag that inflates with 3 moles of N2 at...
Calculate the pressure inside a 20 L airbag that is inflated with 3 moles of N,(g) at 20 °C. О 2.91 О 0.81 o o o o op O 1.61 O3.61 O 2.41
A vehicle airbag uses a gas generator that contains a mixture of three compounds: NaN3, KNO3, and SiO2. A series of three reactions is used to convert the highly toxic sodium azide, NaN3, into N2 gas and harmless silicate glass. The nitrogen gas fills up the airbag, causing it to rapidly expand in a head-on collision. Balance the reactions involved in the deployment of an airbag by inserting the appropriate coefficients. 1. NaN3(s)--> Na(s)+N2(g) 2. Na (s)+ KNO3(s)--> K2O(s)+N2(g) 3....
What pressure (in atm) will 0.52 moles of N2 exert in a 2.6 L container at 25°C?
If I place 10 moles of N2 and 13 moles of CO2 in a 40 L container at a temperature of 25° C, what will the pressure of the resulting mixture of gases be?
1. At STP, 1 mole N2 gas occupies ____________ L, and this accounts for _____________ x 1023molecules and 28.0 ______________ of nitrogen. 2. Calculate the Kelvin temperature to which 10.0 L of a gas at 27 °C would have to be heated to change the volume to 12.0 L. Units of Kelvin are assumed here for the answer you enter so just put the number value. 3. If a plastic container of food at 1.0°C and 750. mmHg is heated...
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) 2 Na(s) +3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaN3 do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) → 2 Na(s) + 3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaNz do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
A bicycle pump inflates a tire whose volume is 515 mL until its internal pressure is 6.30 bar at a temperature of 20.7 oC. a. How many moles of air does the tire contain? b.What volume of air (in L) at 1.01 bar and 20.7 oC did the pump transfer?
A cylinder has a volume of 10.5 L and the pressure of the gas inside is 0.92 atm. By moving the piston, the volume increased to 15.4 L. What is the new pressure? O 0.84 atm 1.3 atm 1.4 atm O 0.63 at A ballon has a volume of 15.5 L at atmospheric pressure and 35°C. What is the new volume if we cool down the ballon to 5.2°C? 2.3L 14.0L 17.2L 14L How many moles of an ideal gas...
How many moles of N2 are in a 2.23 L cylinder at 50.2 °C and 4.59 atm? What pressure is exerted by 814.5 g of CH4 in a 0.730 L steel container at 190.8 K?