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3 years ago

Examples of quantitative of quantitative data

2 answers:

8 0

Answer: Quantitative data is usually collected for statistical analysis using surveys, polls or questionnaires sent across to a specific section of a population.

Here are some example of quantitative data:

A jug of milk holds one gallon.

The painting is 14 inches wide and 12 inches long.

The new baby weighs six pounds and five ounces.

A bag of broccoli crowns weighs four pounds.

hope it helps:)

Zanzabum3 years ago

6 0

Answer:Quantitative data are data which are measured through direct sources of measurements; this means that we can observe them directly and measure them directly with the tools we're using. An example of this would be measuring the length of a football stadium with a measuring tape. Another would be measuring weight with a scale.hope it helps

Explanation:

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3 years ago

Which of the following statements about alkenes is not correct?

professor190 [17]

Option-C: They react mainly by substitution.

Explanation:
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3 years ago

Read 2 more answers

How much heat must your body transfer to 500.0g of water to heat it from 25.0°C to body temperature, 37.0°C?

shtirl [24]

Answer : The heat your body transfer must be, 25.1 kJ

Explanation :

Formula used :

$Q=m\times c\times \Delta T$

or,

$Q=m\times c\times (T_2-T_1)$

where,

Q = heat = ?

m = mass of water = 500.0 g

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

$T_1$ = initial temperature = $25.0^oC$

$T_2$ = final temperature = $37.0^oC$

Now put all the given value in the above formula, we get:

$Q=500.0g\times 4.18J/g^oC\times (37.0-25.0)K$

$Q=25080J=25.1kJ$

Therefore, the heat your body transfer must be, 25.1 kJ

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3 years ago

A sample of H2 gas (2.0 L) at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25 °C i

Tamiku [17]

For this system, we use Dalton's law of partial pressures where the total pressure of a gas mixture is said to be equal to the sum of the partial pressures of the gases. The partial pressure of each gas would be calculated by the product of the mole fraction and the original pressure of the gas. We do as follows:

Total pressure = x1P1 + x2P2
Total pressure = (2.0 / 7.0 )(3.5) + (1.5/7.0)(2.6)
Total pressure = 1.56 atm

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4 years ago