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4 years ago

When are tides highest?

1 answer:

7 0

A neap tide is the highest tide there is, this is due to the position of the moon,since the moon and sometimes the earth are what cause the tides in the ocean.

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(d) If you have 9.44 g of NazPO4, how many grams of AgNO, will be needed for complete

AlladinOne [14]

30.6 g of AgNO₃

Explanation:

We have the following chemical reaction:

Na₃PO₄ + 3 AgNO₃ → Ag₃PO₄ + 3 NaNO₃

Now we calculate the number of moles of Na₃PO₄:

number of moles = mass / molecular weight

number of moles of Na₃PO₄ = 9.44 / 164 = 0.06 moles

Now we formulate the following reasoning:

if 1 mole of Na₃PO₄ will react with 3 moles of AgNO₃

then 0.06 moles of Na₃PO₄ will react with X moles of AgNO₃

X = (0.06 × 3) / 1 = 0.18 moles of AgNO₃

mass = number of moles × molecular weight

mass of AgNO₃ = 0.18 × 170 = 30.6 g

Learn more about:

mole concept

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3 0

3 years ago

4. Suppose 8.00 g of CH4 is allowed to burn in the presence of 16.00 g of oxygen. CH4(g)+2O2(g)-->CO2(g)+2H2O(g)

umka21 [38]

<h3>Answer:</h3>

No masses of CH₄ and O₂ remained after the reaction, while 22.005 g of CO₂ and 18.02 g of H₂O remained

<h3>Explanation:</h3>

The combustion of methane is given by the reaction;

CH₄(g)+2O₂(g) → CO₂(g)+2H₂O(g)

We are given, 8 g of CH₄ and 16.00 g of O₂

Required to determine the mass of CH₄, O₂, CO₂ and H₂O that remained after the complete reaction.

<h3>Step 1: Moles of CH₄ and O₂ in the mass given </h3>

Moles = mass ÷ molar mass

Molar mass of CH₄ = 16.04 g/mol

Moles of CH₄ = 8.00 g ÷ 16.04 g/mol

= 0.498 moles

= 0.5 moles

Molar mass of O₂ = 16.0 g/mol

Moles of O₂ = 16.00 g ÷ 16.00 g/mol

= 1 mole

From the reaction, 1 mole of CH₄ reacts with 2 moles of O₂

CH₄ is the limiting reactant since it is way less than the amount of O₂

Therefore, 0.5 moles of CH₄ will react with 1 mole of oxygen.

This means there will be no amount of O₂ and CH₄ that remains.

<h3>Step 2: Moles of CO₂ and H₂O that were produced.</h3>

From the reaction 1 mole of CH₄ reacts with 2 moles of O₂ to produce 1 mole of CO₂ and 2 moles of H₂O.

Therefore,

In our case, 0.5 moles of CH₄ will react with 1 mole of O₂ to produce 0.5 moles of CO₂ and 1 mole of H₂O.

<h3>Step 3: Mass of CO₂ and H₂O produced </h3>

Mass = Moles × Molar mass

Molar mass of CO₂ = 44.01 g/mol

Mass of CO₂ = 0.5 mol × 44.01 g/mol

= 22.005 g

Molar mass of H₂O = 18.02 g/mol

Moles of H₂O = 1 mole × 18.02 g/mol

= 18.02 g

Therefore, no masses of CH₄ and O₂ remained after the reaction, 22.005 g of CO₂ and 18.02 g of H₂O remained

3 0

4 years ago

Read 2 more answers

What is the mass of 1.2x10^25 atoms of Helium

Molodets [167]

Answer:

dunno

Explanation:

sorry

4 0

3 years ago

Period 6, group 12 (2B)

maksim [4K]

Answer:

mercury or Hg

Explanation:

i looked at the periodic table haha

hope this helps and is right <3

6 0

4 years ago

Be sure to answer all parts. Determine the overall orders of the reactions to which the following rate laws apply: (a) rate = k[

Svetach [21]

Answer :

(a) The rate of reaction is, second order reaction.

(b) The rate of reaction is, zero order reaction.

Explanation :

Rate of reaction : It is defined as the rate of change in concentration of reactant or product with respect to time.

Order of reaction : It is defined as the sum of the exponents or powers to which the molar concentration in the rate law equation are raised to express the observed rate of reaction.

The order of reaction depends on the power of reactant concentration.

(a) The given rate expression is,

$Rate=k[NO_2]^2$

From this expression we conclude that the power of concentration of reactant $NO_2$ is 2.

That means it is a second order reaction.

(b) The given rate expression is,

$Rate=k$

From this expression we conclude that the rate of reaction is equal to rate constant.

That means it is a zero order reaction.

4 0

3 years ago