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3 years ago

Which group of elements will form molecular compounds? (Choose all that apply)

Chemistry

1 answer:

AlekseyPX3 years ago

8 0

Carbon & Hydrogen
I don’t see your answer choice

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An ideal gas in a sealed container has an initial volume of 2.65 L. At constant pressure, it is cooled to 25.00 ∘C, where its fi

svet-max [94.6K]

Answer:

Initial temperature was: $178.3^\circ \:C$

Explanation:

The Relation between the volume and temperature at constant pressure is:

$\frac{V_1}{T_1}=\frac{V_2}{T_2}\\\\\frac{2.65}{T_1}=\frac{1.75}{\left(25+273\right)}\\\\T_1=451.3\:K\quad\:or\:\quad 178.3^\circ\:C$

8 0

4 years ago

What mass of oxygen forms from 71.89 g CO2? Use the periodic table to find molar masses.

Paraphin [41]

Atomic mass C = 12.0107
Atomic mass O= 15.9994
Calculate the molecular mass of the CO2
12.0107 + (2 x 15.9994) = 44.0095

Multiply the mass of CO2 by the conversion factor that relate the O mass to the molecular mass of CO2 to find the mass of O in the 71.89g of CO2

71.89 g CO2 x (2 x 15.9994) / 44.0095 =

52.2703900748702

52.27 g O

8 0

4 years ago

What are most conductors made of? A: Wood B: Paper C: Plastic D: Metal

mafiozo [28]

Answer:

D: Metal

Explanation:

Most conductors are made from metal, for the alloys allow for a "freer" passage way for electrons to pass through.

7 0

3 years ago

Read 2 more answers

I am having trouble solving it pls help

MAXImum [283]

Answer:

1. 0.097 s

2. 0.420 M

Explanation:

To solve both questions we'll use the formula:

[A]ₓ = [A]₀ - kt

Where [A]ₓ is the concentration of A at a given time; and [A]₀ is the initial concentration.

1) We input the data given by the problem:

0.167 M = 0.700 M - 5.48 M/s * t

And solve for t:

t = 0.097 s

2) We input the new data:

[A]ₓ = 0.500 M - 0.361 M/s * 0.220 s

and solve for [A]ₓ:

[A]ₓ = 0.420 M

5 0

3 years ago

2. 1.5 moles of AgNO3 reacts with 0.5 mole of Mg3P2. Calculate the moles of excess

kicyunya [14]

Answer:

No of Moles in excess at the end of the reaction is 0.25 moles

Explanation:

AgNO3 + Mg3P2 → Ag3P + Mg(NO3)2

Balancing the equation we get

6AgNO3 + Mg3P2 → 2Ag3P + 3Mg(NO3)2

6 moles of AgNO3 needs 1 mole of Mg3P2

using unitary method

AgNO3 = $\frac{1}{6}*Mg3P2$

1.5 AgNO3 = $\frac{1}{6}*1.5$

= 1/4 = 0.25moles of Mg3P2

So 1.5 Moles of AgNO3 requires 0.25Mg3P2 for complete reaction but we have 0.5Moles of Mg3P2 available Therefore Mg3P2 is in excess

No of Moles in excess at the end of the reaction = 0.5 - 0.25 = 0.25moles

5 0

3 years ago