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3 years ago

How does a physical change differ from a chemical change

Chemistry

2 answers:

gtnhenbr [62]3 years ago

7 0

A chemical change is something you can't see and a physical change is something you can see.

inysia [295]3 years ago

6 0

With a physical change you can actually see it change like ice turning into water, then with a chemical change you can't see it change, although within the molecules themselves they change which makes that possible.

Hope this helps!

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Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water. P

pantera1 [17]

Answer:

The mass of P₄O₁₀ (s) formed is 471.03 g

Explanation:

4PH₃(g) + 8O₂(g) → P₄O₁₀ (s) + 6H₂O (g)

This is the ballanced equation.

Every 4 moles of phosphine, 1 mol of tetraphosphorus decaoxide is generated.

Moles of PH₃ = Mass PH₃ / Molar mass PH₃

Moles PH₃ = 225 g / 33.9 g/m

Moles PH₃ = 6.63 moles

So the rule of three, will be:

If 4 moles of PH₃ generate 1 mol P₄O₁₀

Then, 6.63 moles of PH₃ generate (6.63 .1)/4 = 1.66 moles

If we want to know the mass:

Moles . Molar mass = mass

Molar mass P₄O₁₀ = 283.88 g/m

1.66m . 283.88 g/m = 471.03 g

3 0

3 years ago

Organisms are more closely related to the species that they share the most DNA with

Aleonysh [2.5K]

Answer:

True

Explanation:

3 0

3 years ago

What volume will 2.35 moles of nitrogen gas, at STP, occupy?

snow_tiger [21]

Answer:

STP of 1atm and 273 k for pressure

4 0

2 years ago

** worth 20 points + brainliest **

Bad White [126]

Answer : The correct option is, (D) $83^oC$

Solution :

Formula used :

$Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})$

where,

Q = heat released = -1300 J

m = mass of water = 40 g

c = specific heat of water = $4.18J/g^oC$

$\Delta T=\text{Change in temperature}$

$T_{final}$ = final temperature = ?

$T_{initial}$ = initial temperature = $91.0^oC$

Now put all the given values in the above formula, we get the final temperature of water.

$-1300J=40g\times 4.18J/g^oC\times (T_{final}-91.0^oC)$

$T_{final}=83.2^oC\approx 83^oC$

Therefore, the final temperature of the water is, $83^oC$

5 0

3 years ago

What is the volume of solution (in mL) produced when 91.80g of Mg(OH)2 are used

hram777 [196]

Answer: The volume of solution is 2248 ml

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

$Molarity=\frac{n\times 1000}{V_s}$

where,

n = moles of solute

$V_s$ = volume of solution in ml

moles of $Mg(OH)_2$ = $\frac{\text {given mass}}{\text {Molar mass}}=\frac{91.80g}{58.32g/mol}=1.574mol$

Now put all the given values in the formula of molality, we get

$0.7=\frac{1.574\times 1000}{V_s}$

$V_s=\frac{1.574\times 1000}{0.7}=2248ml$

Therefore, the volume of solution is 2248 ml

4 0

2 years ago