well it saids:

A 1.50L rubber balloon is filled with carbon dioxide gas at a temperature of 0.00C and a pressure of 1.00 atm. the density of the carbon dioxide gas under these conditions is 1.98g/L.

a)at 50.0C the balloon ha a vlomue of 1.78L. Calculate the carbon dioxide density at this temperature.

I would use

p*molar mass CO2 = density(g/L) CO2*R*T

To answer this question, you need to use the ideal gas law and the ideal gas equation. The ideal gas equation is given by:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature

The ideal gas constant, R, has a value of 0.0821 L·atm/(mol·K).

To calculate the carbon dioxide density at 50.0°C, we need to find the number of moles of carbon dioxide gas and divide it by the volume of the balloon.

Step 1: Convert the given temperature to Kelvin (K).
T = 50.0°C + 273.15 = 323.15 K

Step 2: Use the ideal gas equation to calculate the number of moles of carbon dioxide gas.
PV = nRT
n = PV / RT

Given:
P = 1.00 atm
V = 1.78 L
T = 323.15 K
R = 0.0821 L·atm/(mol·K)

n = (1.00 atm * 1.78 L) / (0.0821 L·atm/(mol·K) * 323.15 K)

Step 3: Divide the number of moles by the volume to get the density of carbon dioxide gas.
Density = n / V

So, once you have the value of n (number of moles) from Step 2, you can divide it by the given volume (1.78L) to find the carbon dioxide density at 50.0°C.