Question

At a temperature of 252.4°C, the
average velocity (meters / second) of a propane,
C_{3}H_{8}, molecule is:

(a) 2.973 x 10^{5}
m/s (b) 461.0
m/s
(c) 545.2
m/s
(d) 418.1 m/s

Answer #1

Please find the attachment.

Propane (C3H8) is burned with excess air, both supplied at 25C.
Assume that air is 21% oxygen, balance nitrogen.
Part 1 : If 1.0 mol of propane is burned with x mols of air, how
many mols of oxygen appear in the combustion products?
A. 3.0 + 0.21x
B. 4.0 + 0.79x
C. 0.79x
D. 0.21x – 5.0 .
Part 2 : The standard heat of combustion for propane
A. depends on the state of the water in the products...

Propane (C3H8) boils at ‐42.0 °C with a heat of vaporization of
19.0 kJ/mol. Calculate the heat involved in bringing 50.0 mL of
liquid propane at ‐50.0° C to 20.0 °C.
Data: liquid propane density = 2.01
g/cm3, specific heat capacity of liquid propane = 1.32 J g‐1 °C‐1 ,
specific heat capacity of gaseous propane = 1.64 J g‐1 °C‐1 .
Assume heat capacity does not vary with temperature.

Suppose you toss a basketball upward while standing still with
an initial velocity of 7 meters/second and it rises to about 2.45
meters. That's below the standard 3.05 meters (10 feet) for a
basketball hoop, so you miss the shot. Which of these would get you
the goal
a)
Give the same 7 m/s from the same height, but early in a jump
upward at 1 m/s.
b)
From standing still, give a velocity of 8 m/s.
c)
Give the...

#6 The following reaction shows combustion reaction of propane
gas at 25 Celsius.
C3H8(gas)+5O2(gas)<===>
3CO2(gas)+4H20(liq);
deltaH=-2219.97 kJ/mol
Initially 1L-chamber contained 2.03M of propane
(C3H8), 3.50 M of oxygen (O2) and
0.030M of carbon dioxide (CO2). After equilibrium is
reached, the chamber contained 1.53 M of propane
(C3H8).
a)Using the information given,calculate equlibrium constant
(Kc) of thid reaction.
b) After equilibrium is reached, if the chamber size is
increased to 5L, predict the direction of equilibrium shift.
Explian your answer.
c)After...

For water at the room temperature, the velocity of a molecule of
food color is about 0.8x104 cm/s and the mean free path
is on the order of 10-8 cm. Calculate the
time required to displace this molecule by 0.75x10-3 cm.
Assume that the diffusion is independent of the mass of this
molecule. Notation: 10^n is equivalent to 10n
0.005 s
0.08 s
0.01 s
0.007 s
10 x 10^-3 s
6 s
10000 s
0.7 s

Industrially, hydrogen gas can be prepared by combining propane gas
(C3H8) with steam at about 400°C. The
products are carbon monoxide gas (CO) and hydrogen gas
(H2).
(a) Write a balanced equation for the reaction.
(b) How many kilograms of H2 can be obtained from 3.95
×103 kg of propane?
____×10____kg H2 gas

The average speed of a diatomic oxygen molecule at 25 ∘C is
482.1 m⋅s−1 . What is the average wavelength of an oxygen molecule
at this temperature? Assume that the molecule acts as a single
particle.

A
0.50 kg cart with a velocity of 2.0 meters per second collides with
a 1.0 kg cart which is motionless. Just after the collision the
second cart has a velocity of 1.2 meters per second. (Neglect
friction) a) what will be the velocity of the 0.50 kg cart just
after the collision? b) what per cent of the original energy is
lost in the collision?

The velocity function (in meters per second) is given for a
particle moving along a line.
v(t) =
t2 − 2t −
8, 1 ≤ t ≤ 5
(a) Find the displacement. (m)
(b) Find the distance traveled by the particle during the given
time interval. (m)

At 20 ∘C (approximately room temperature) the average velocity
of N2 molecules in air is 1050 mph.
Part A What is the kinetic energy (in J) of an N2 molecule
moving at this speed? Express your answer using four significant
figures.
Part B What is the total kinetic energy of 1 mol of N2 molecules
moving at this speed? Express your answer using four significant
figures.

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