Ask question

Ask question

All categories

3 years ago

7

Four balls have the same temperature. Which ball has the most Thermal Energy? A.Golf ball(45g) B.Basket ball(625g) C.Bowling bal

l(5000g) D.Tennis ball(60g)

1 answer:

Nonamiya [84]3 years ago

4 0

Answer:

b

Explanation:

b. ,u play with the ball, handle the ball grab the ball throw the ball exc.

You might be interested in

If 3.5 mols of P2O3 are formed, how many<br> moles of P4 reacted?

EleoNora [17]

P2 is 3.5 for p4= 2p2 i.e 2*3.5=7

8 0

3 years ago

Read 2 more answers

A homogenous mixture (is, is not) uniformly distributed

Solnce55 [7]

Answer:

In a homogeneous mixture, there is uniform distribution of particles.

${}$

3 0

2 years ago

HELP! PLEASE! ASAP! Manganese(III) fluoride, MnF3, can be prepared by the following reaction:

Crank

Answer:

14.336 g MnF₂

Explanation:

number of moles = mass / molecular weight

number of moles of MnI₂ = 55 / 309 = 0.178 moles

number of moles of F₂ = 55 / 38 = 1.447 moles

From the reaction and the number of moles calculated we deduce that the fluorine F₂ is a limiting reactant.

So:

if 13 moles of F₂ reacts to produce 2 moles of MnF₃

then 1.447 moles of F₂ reacts to produce X moles of MnF₃

X = (1.447 × 2) / 13 = 0.223 moles of MnF₃ (100% yield)

For 57.2% yield we have:

number of moles of MnF₃ = (57.2 / 100) × 0.223 = 0.128 moles

mass = number of moles × molecular weight

mass of MnF₃ = 0.128 × 112 = 14.336 g

3 0

3 years ago

Gaseous compound Q contains only xenon and oxygen. When 0.100 gg of Q is placed in a 50.0 mLmL steel vessel at 0 ∘C∘C, the press

asambeis [7]

The question is incomplete, here is the complete question:

Gaseous compound Q contains only xenon and oxygen. When a 0.100 g sample of Q is placed in a 50.0-mL steel vessel at 0°C, the pressure is 0.229 atm. What is the likely formula of the compound?

A. XeO

B. $XeO_4$

C. $Xe_2O_2$

D. $Xe_2O_3$

E. $Xe_3O_2$

<u>Answer:</u> The chemical formula of the compound is $XeO_4$

<u>Explanation:</u>

To calculate the molecular mass of the compound, we use the equation given by ideal gas equation:

PV = nRT

Or,

$PV=\frac{w}{M}RT$

where,

P = Pressure of the gas = 0.229 atm

V = Volume of the gas = 50.0 mL = 0.050 L (Conversion factor: 1 L = 1000 mL)

w = Weight of the gas = 0.100 g

M = Molar mass of gas = ?

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = Temperature of the gas = $0^oC=273K$

Putting value in above equation, we get:

$0.229\times 0.050=\frac{0.100}{M}\times 0.0821\times 273\\\\M=\frac{0.100\times 0.0821\times 273}{0.229\times 0.050}=195.4g/mol\approx 195g/mol$

The compound having mass as 195 g/mol is $XeO_4$

Hence, the chemical formula of the compound is $XeO_4$

5 0

3 years ago

1. Rank the following solutions in order of increasing

babunello [35]

The order of the solutions from lowest to highest concentration : A, B, C

<h3>Further explanation</h3>

Given

the following solutions

Required

order of increasing concentration

Solution

Molarity shows the number of moles of solute in every 1 liter of solution.

$\large{\boxed {\bold {M ~ = ~ \frac {n} {V}}}$

Solution A : 0.5 moles : 2 L solution = 0.25 M

Solution B : 1 moles : 3 L solution = 0.33 M

Solution C : 1.5 moles : 4 L solution = 0.375 M

8 0

3 years ago